For the aqueous reaction dihydroxyacetone phosphate is the reactant and glyceraldehyde 3 phosphate is the product. dihydroxyacetone phosphate − ⇀ ↽ − glyceraldehyde − 3 − phosphate the standard change in Gibbs free energy is Δ G ° ' = 7.53 kJ/mol . Calculate Δ G for this reaction at 298 K when [dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00400 M . Δ G = kJ / mol

Answer : The Gibbs free energy of the reaction is -0.445 kJ/mol.

Explanation :

The given chemical equation is:

The expression for of above equation is:

Given:

[Glyceraldehyde-3-phosphate] = 0.00400 M

[Dihydroxyacetone phosphate] = 0.100 M

Now put all the given values in above equation, we get:

The relation between standard Gibbs free energy and equilibrium constant follows:

where,

= Standard Gibbs free energy = 7.53 kJ/mol = 7530 J/mol

(Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314J/K mol

T = temperature = 298 K

Now put all the given values in above equation, we get:

Hence, the Gibbs free energy of the reaction is -0.445 kJ/mol.

your answers are a,b,,e and f

i hope this

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